Lecture 7: Ionic Bonding Flashcards
What is a chemical bond?
An attractive force that holds two or more atoms together
What are the four types of chemical bonds?
- Ionic
- Covalent
- Dative
- Metallic
What do most atoms adjust their valence shells to?
8 e-
Which atoms do not obey the 8 e- rule?
Transition metals using their d-orbitals (they use the 18 e- rule)
How will a proton act on another proton?
They will repel
How will an electron act on a proton?
They will attract
How will a neutron act on an electron?
It will not
How is the force acting on each particle linked to the size of the charge?
(HINT: Columb’s Law)
They are proportional
How is the force acting on each particle linked to the distance between them?
(HINT: Coulomb’s Law)
Inverse square
What is electronegativity?
The ability of an atom to attract electrons in a chemical bond
What factors affect electronegativity?
- The charge of the nucleus
- Atomic radius
- Screening (shielding)
Which element is most electronegative?
Why?
Fluorine
Small atomic radius, high nuclear charge
Explain ionic bonds
Bonds between metals and non-metals
Metals donate electrons
Non-metals gain electrons
This forms oppositely-charged ions
The ions then attract each other
Describe the properties of an ionic bond (4+1)
- Non-directional
- The compound will dissolve and dissociate in polar solvents
- (the separated ions are solvated)
- The bonds can be broken by melting
- The compounds have no overall charge
Which factors favour ionic bonding? (6)
- Low IE of the metal
- High EA of the non-metal
- Small non-metal
- Low anion charge
- Large electronegativity difference between the ions
- High lattice energy
